What are Isotopes?

The term isotope is derived from the Greek words isos (“equal”) and topos (“place”), which signify “the same location.” As a result, different isotopes of a single element occupy the same spot on the periodic table. Margaret Todd, a Scottish doctor and journalist, suggested the term to chemist Frederick Soddy in 1913.

Isotopes

Isotopes are atoms of a chemical element that have the same atomic number and location in the periodic table as well as almost identical chemical activity but differ in atomic weights and physical attributes. There are one or more isotopes for every chemical element.

The number of protons in an atom’s nucleus is used to identify and label the atom. This atomic number is usually denoted by the letter Z. The significance of the atomic number stems from the fact that all atoms with the same atomic number have chemical properties that are substantially, if not exactly, identical. A sample of an element is a big group of atoms with the same atomic number.

Facts About Isotopes

• Isotopes exist in all elements.
• Stable and unstable isotopes are the two primary categories of isotopes (radioactive).
• There are 254 stable isotopes known.
• Scientists call artificial (lab-made) isotopes radioisotopes because they are unstable and so radioactive.
• Some elements can only exist in a state of instability (for example, uranium).
• Deuterium (hydrogen with one neutron) and tritium (hydrogen with two neutrons) are the only isotopes of hydrogen with distinct names.

Uses of Isotopes

• Cobalt-60 emits gamma rays, which can be employed in cancer treatment.
• Less penetrating radiation from strontium-90 or phosphorus-32 is used to treat superficial tumors like skin cancer.
• A heart pacemaker containing plutonium-238 can be used to help patients with heart issues control their heartbeats.
• Thyroid therapy with iodine 131 is possible.
• Carbon-14 is used to determine the age of bones, fossils, and wood by determining how much carbon-14 is present.

Isobars

Isobars are chemical elements with the same atomic mass but an unique atomic number. The atomic mass is the sum of the protons and neutrons. As a result, the atomic mass of an atom is equal to the number of nucleons contained in the nucleus. It would have the same number of nucleons as the previous one.

Although the number of protons and neutrons will vary, the number of nucleons, or the sum of protons and neutrons in isobars, will remain constant. Because of the difference in atomic numbers, isobars always have different atomic structures. The disparity in the number of nucleons is compensated for by the amount of neutrons. As a result, they are always distinct chemical elements with the same atomic mass.

Uses of Isobars

• Uranium isobars may be used in nuclear reactors.
• Goiter is treated with iodine isobar.
• Cancer can be treated with cobalt isobaric.

Radioactive Isotopes

Any of numerous species of the same chemical element with differing masses whose nuclei are unstable and expend surplus energy by randomly emitting radiation in the form of alpha, beta, and gamma rays, also known as radioisotope, radionuclide, or radioactive nuclide.

There are one or even more radioactive isotopes for every chemical element. The lightest element, hydrogen, has 3 isotopes with mass numbers 1, 2, and 3. The only radioactive isotope is hydrogen-3 (tritium), whereas the other two are stable. There are about 1,000 radioisotopes of various elements. Only about 50 of these are found naturally; the rest are created intentionally as direct products of nuclear processes or as radioactive descendants of these products.

Conclusion

Radioactive isotopes of various sorts are used in industry to measure the thickness of plastic or metal sheets; the strength of the radiant energy that penetrates the material being investigated indicates the precise thickness. They could also be used to inspect fabricated metal parts for structural flaws instead of huge X-ray machines.